The reaction of tert-butyl bromide, (CH3)3CBr, with methanol (base) proceeds by an E1 mechanism. What is the effect of doubling the concentration of methanol (base)? O The rate remains the same O The rate decreases by a factor of 2 O The rate increases by a factor of 2 O The rate increases by a factor of 4

The reaction of tert-butyl bromide, (CH3)3CBr, with methanol (base) proceeds by an E1 mechanism. What is the effect of doubling the concentration of methanol (base)? O The rate remains the same O The rate decreases by a factor of 2 O The rate increases by a factor of 2 O The rate increases by a factor of 4

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 58E: Theophylline is a pharmaceutical drug that is sometimes used to help with lung function. You observe...

See similar textbooks

Similar questions

You and a coworker have developed a molecule thathas shown potential as cobra antivenin (AV). This antivenin works by binding to the venom (V), thereby rendering it nontoxic. This reaction can be described by the rate law Rate=k[AV]1[V]1 You have been given the following data from your coworker: [V]0=0.20M[AV]0=1.0104M A plot of ln[AV] versus t(s) gives a straight line with a slope of 0.32 s1. What is the value of the rate constant (k) for this reaction?
1. The following data were collected from the alkaline hydrolysis reaction of t-butylbromide to t-butyl alcohol as: (CH3)3CBr à alkaline hydrolysis à (CH3)3COH a. At concentration 0.5 M the rate was 0.005 (mol/L.s) b. At concentration 1.5 M the rate was 0.015 (mol/L.s) If you know that: Rate2 / Rate1 = ([A2] / [A1])m Find out the followings: a. The reaction order b. The reaction constant c. The half-life of the reaction.
Suppose the formation of tert-butanol proceeds by the following mechanism: step elementary reaction rate constant 1 CH33CBr (aq) → CH33C+ (aq) + Br− (aq) k1 2 CH33C+ (aq) + OH− (aq) → CH33COH (aq) k2 Suppose also k1 ≫ k2 . That is, the first step is much faster than the second.
Doubling the concentration of hydroxide ions in the following reaction causes the reaction rate to double. Doubling the concentration of both reactants causes the reaction rate to increase by a factor of four. C 2 H 5 Br (aq) +OH ^-(aq) ----> C 2 H 5 OH (aq) +Br^ - (aq) a) What is the order of the reaction with respect to hydroxide ions? b) What is the order of the reaction with respect to bromoethane ? c) What is the overall reaction order?
Table 1 with temperature and rate constants Temperature (oC) Rate constants KH (min-1) 61.0 7.13*10-6 71.2 2.77*10-5 Mark and Anthony have considered the following reaction for urea NH2CONH2 in 0.1M HCl: NH2CONH2 + 2H2O --> 2NH+2 + CO2-3 and the rate constant for the reaction is k1. Stephan and Kurt have been in the laboratory and measured rate constants for the reaction at two different temperatures. The measurement results are given in Table 1. 1) You must write down expressions for the changes in time for the concentrations of the reactants and products. That is, determine d[X]/dt, where [X] is the concentration of either reactants or products and write this down using concentrations and the rate constant. 2) You must use the Arrhenius expression to determine the activation energy for the reaction. 3) You must use the Arrhenius expression to determine the pre-exponential factor in the Arrhenius expression.
The following reaction mechanism was proposed for this reaction: (1) To2 → 2To [slow] (2) 2To + O2 → 2ToO [fast] (3) 2ToO + To2 → 2To2O [fast] What would be the molecularity of step? Would this be a possible mechanism for this reaction? Explain
The reaction below has rate constant 2.50 x 10 -1 min -1 and obeys the rate law: rate = k [A]. At what time will 61.9 % of A have reacted? A --> B The reaction below has rate constant 2.50 x 10 -1min -1 and obeys the rate law: rate = k [A]. At what time will 61.9 % of A have reacted? A --> B 80.8 min 16.9 min 0.00114 min 0.567 min 0.0601 min 3.85 min 19.8 min 495 min
What is the average rate of the reaction from t1=0 s to t2=50 s
Consider the chemical reaction described by 2A(aq) ⇌ D(aq)with rate constants k1 and k-1. If k1 = 5.9×10-5 Lmol-1s-1 and Keq = 0.27 what is k-1 for a solution originally prepared with [A]0 = 0.123 molL-1 and [D]0 = 0?
A + 2B -> C (rate constant = k1, rA = -k1[A][B]2) C -> A + 2B (rate constant = k-1, rA = k-1[C]) C + 2A -> 2D (rate constant = k2, rA = -k2[C][A]2) reaction rate constant and the rate for A of each elementary reaction are shown in the parentheses after each reaction. Calculate the overall reaction rate for A in terms of [A], [B], k1, k-1, and k2 assuming c is psuedo-state-concentration overall chemical rxn is 3A+2B->2D
The second-order rate constant for the reaction CH3COOC2H5(aq) + OH-(aq)→ CH3CO2-(aq) + CH3CH2OH(aq) is 0.11 dm3 mol-1 s- 1. What is the concentration of ester after(a) 15 s, (b) 15 min when ethyl acetate is added to sodium hydroxide so that the in it ial concentrations are [NaOH] 0.055 mol dm-3 and [CH3COOC2H5] = 0.150 mol dm-3?
rate law for hte reaction : RX + H20→ R0H + HX , rate =K[RX]. the rate of reaction will be doubled when: (a) concentration of H2O is doubled (b)concentration of RX is reduced to half (c) concentration of RX is doubled (d) none of these also give reason for your answer